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MHT-CET : Chemistry Entrance Exam

MHT - CET : Chemistry - Ionic Equilibria Know More

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1. Acid Base Concept
All Bronsted bases are also Lewis bases but all Bronsted acids are not Lewis acids. According to Bronsted concept, a base accepts proton whereas Lewis concept says that a base is a substance which donates electron pair. Lewis bases contain one or more lone pair of electrons and therefore can accept a proton (Bronsted base). Thus, all Lewis bases are also Bronsted bases. But all Bronsted acids are not Lewis acids. Bronsted acids are those which can give a proton. Example: HCl, H2SO4 are Bronsted acids but they are not capable of accepting electron pair.

2. Effect of Temperature on Kw
The values of [H3O+] and [
OH-] are always equal at all temperatures but values of Kw are different at different temperatures.
Value of Kw increases with rise in temperature, which can be understood on the basis of Le - Chatelier's principle.

2H2O(l) H3O+(aq) +OH-(aq)

D H = + 57.3 kJ.


Increase in temperature will shift the equilibrium in forward direction producing larger concentration of H3O+ and OH- ions. Hence, Kw increases with rise in temperature.

3. Comparison of Solubility Product and Ionic Product

 

Solubility Product

 

Ionic Product

1.

It is the product of concentration of ions of the electrolyte, raised to the power of their coefficients in balanced chemical equation in a saturated solution.

1.

It is the product of concentration of ions of the electrolyte raised to the power of their coefficients in balanced chemical equation in solution at any concentration.

2.

For an electrolyte at a constant temperature, it has a constant value.

2.

The value does not remain constant and varies with change in concentration.


4.
Henderson's Equation

For acidic buffers

pH = pKa + log

[salt]

[Acid]

where PKa =

- Log Ka

For basic buffers

 

pOH = pKb + log

[salt]

[Base]

or PH = 14- pKb - log

[salt]

[Base]

Where Pkb = - log Kb

 

 

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